Final answer:
To determine the molarity of a barium hydroxide solution, we can use the results of its titration with hydrochloric acid. Given the volume of barium hydroxide and hydrochloric acid, and the molarity of the latter, we apply the titration formula and consider the mole ratio to calculate the molarity of the barium hydroxide, which is determined to be 1.4 M.
Step-by-step explanation:
To find the molarity of the barium hydroxide solution, we use the concept of titration. In titration, the molarity (M1) of one solution is used to find the molarity of another solution by using the volume (V1) of the first solution, the volume (V2) of the second solution, and the molarity (M2) of the second solution.
In this case, barium hydroxide (Ba(OH)2) reacts with hydrochloric acid (HCl) in a 1:2 mole ratio because a single unit of barium hydroxide can react with two units of hydrochloric acid. The balanced equation for this reaction is:
Ba(OH)2(aq) + 2 HCl(aq) → BaCl2(aq) + 2 H2O(l)
The given values are: V1 (volume of barium hydroxide) = 25 mL or 0.025 L, M2 (molarity of HCl) = 0.1 M, V2 (volume of HCl) = 35 mL or 0.035 L.
Using the titration formula: M1V1 = M2V2/n, where n is the mole ratio of HCl to Ba(OH)2, which is 2, we calculate the molarity of barium hydroxide (M1) as follows:
M1 = (M2 × V2) / (V1 × n)
M1 = (0.1 M × 0.035 L) / (0.025 L × 2) = 0.07 M / 0.05 = 1.4 M.
Therefore, the molarity of the barium hydroxide solution is 1.4 M.